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Will turn into a liquid at room temperature. Off the Periodic Table pick three solid elements that would float when placed in mercury as well as three elements that would sink when placed in mercury.
what is the minimum rate that fresh air has to be supplied to the room so that the concentration of CO2 in the room doesn't exceed 0.500% by mole? Assume the room is well mixed, and the volume of the solid dry ice does not change. mol air/min
Based on the value obtained in the three heating above, do you think the student should have confidence in his results? why? what do you think he should do to be more confident in his result
What mass of sodium phosphate would have to be added to 2.0 of this solution to completely eliminate the hard water ions? Assume complete reaction.
Making plastic drinking bottles for bottled water requires about 58 million barrels of oils per year (2007). In 2007, 300 million people averaged 114 L of bottled water per person. The average cost of 0.6 L was $1.00. The average charge for tap wa..
A solution is prepared by mixing 50.0 mL of 0.11 M Pb(NO3)2 with 50.0 mL of 1.3 M KCl. Calculate the concentrations of Pb2+ and Cl - at equilibrium. Ksp for PbCl2(s) is 1.6* 10-5.
A second sample of this acid weighing 2.00 grams is added to the titrated sample and the pH is 4.32. Calculate the molar mass of the unknown acid and determine the value of Ka for this acid.
Given the amount of alumina to be used, 4g compute the height of alumina in a column with a 1.00 cm diameter. Density of alumina is 0.9 g/ml.
consider 1.0 liters of an aqueous solution that contains 0.10 m sulfuric acid to which 0.30 moles of barium nitrate is
Identify the compounds present in the mixture and determine the percent by mass of each in the original sample. 1 Identity and % (wt/wt)= 2 Identity and % (wt/wt)=
Balance the following equations and write balanced net ion for each reaction. a) HBR(aq) + Ca(OH)2 (aq) b) net ionic equation C) Fe(OH)3 (aq) + H2SO4 (aq) d) net ionic quation
Calculate the hydronium-ion concentration and the pH of a 0.0059 M solution of chloroacetic acid. Ka is 1.3 10-3.
A 15 mL sample of 0.100 M Ba(OH)2 is titrated with 0.12M HCl. Calculated the equivalency point, and the pH after 5mL, 10 mL, 15 mL, and 20 mL of HCl are added.
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